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Question

The nuclear charge actually experienced by an electron is termed as the effective nuclear charge. The effective nuclear charge Z* actually depends on the type of shell and orbital in which electron is actually present. The relative extent to which the various orbitals penetrate the electron clouds of other orbitals is s>p>d>f (for the same value of n)
The phenomenon in which penultimate shell electrons act as screen or shield in between nucleus and valence shell electrons and thereby reducing nuclear charge is known as shielding effect. The penultimate shell electrons repel the valence shell electron to keep them loosely held with the nucleus. It is thus evident that more is the shielding effect, lesser is the effective nuclear charge and lesser is the ionization energy.
Ionization energy is not influenced by :

A
Size of atom
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B
Effective nuclear charge
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C
Electrons present in inner shell
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D
Change in entropy
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Solution

The correct option is B Change in entropy
Change in entropy has no effect on ionization energy.
But as radius decreases, IE increases and also as e
ffective nuclear charge increases, IE increases.

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